In this investigation I am going to be investigating the reaction between marble chips and hydrochloric acid, and to see what differences in the rate of this reaction arise when different concentrations of acid are used. Below is the word equation for this reaction:

The aim of this investigation is to find out whether the concentration of the acid affects the rate of reaction between the acid and marble chips.

Prediction

I predict that, as the concentration of acid in the test tube increases, so too will the rate of reaction. I think this because concentration relates to the amount of molecules in the acid, and if there is a higher concentration of acid there is a larger amount of hydrogen chloride molecules in the acid and therefore they are more likely to collide and react with the calcium carbonate ions present in the marble chips. I would expect the following graph to emerge from the results:

Plan

Before I begin my real experiment, I had to do some preliminary testing. Firstly I set up the apparatus exactly as it would be in the proper experiments. Secondly I experimented with the mass of marble chips and amount of acid used in the experiments. I decided to use acid concentrations ranging from 0.5Mol to 2Mol, and increasing in 0.5Mol increments. The marble chips were measured out into masses of 1.5g. In this preliminary test I measured the amount of gas released in the reaction every thirty seconds for three minutes. Below is the table of results for this preliminary test:

The table shows me that the method of timing these results is sufficient. However, I have realised that I will need to add some concentrations because of the lack of points available for the final graphs. Since the maximum concentration of acid allowed is 2mol, I am going to reduce the incremental value to 0.25mol; therefore giving me the concentrations 0.5mol, 0.75mol, 1mol, 1.25mol, 1.75mol, and 2mol. I am confident that these concentrations will give me sufficient results for my final graphs, so I feel there is no need for further preliminary testing.

Safety Precautions

There are only a few safety precautions relevant to this experiment, giving its relative docility. These are:

Keep long hair and ties tied back/under a jumper;
Push bags under desks & keep the floor clear;
Do not contaminate/mix/spill the acids;
Make sure equipment is securely in place.

Arrangement of Apparatus

Below is the illustration for the way my apparatus is going to be set up for the experiment.

Measurements

I am going to measure the amount of gas released over 3 minutes, taking measurements every thirty seconds. I will read the values off of the gas measuring cylinder, repeating the experiment three times to give me three results for each concentration. Then, after these have been recorded, I will take an average of these results to give me one averaged result. Fair Testing

In the interests of fair testing, I am going to do a few things. These include:

Keeping the mass of marble chips stable at 1.5g for every stage of the experiment; Try not to let the room temperature vary too much to make an impact on my results; Use the same amount of hydrochloric acid (10ml) for every reaction.

The Final ExperimentI am now going to conduct my real experiment, after obtaining sufficient information from the preliminary tests to have a more precise idea of the experiment. Here is the table of results for my experiment:

...Chemestry Lab
Rates of Reaction
(Picture from: http://sciencespot.net/Pages/kdzchem.html)
The rate of reaction is how fast or slow a reaction is completed. This is important for factories and chemists all over the world. What happenes during a reaction is atoms or molecules that collide and form new molecules. You can affect this rate of reaction with: temperature of reactants or suroundings, surface area of reactants, if there is a catalyst present, but in theis lab the concentration was changed as the IV. The reactionrate is masured in change/time, in this case it was: volume of gass produced/minutes. Gas was measured in ml/minute, and this was the DV.
Aim of lab was: To find the change in rate if reaction, depending on the concentration of hydrocloric acid.
Hypothesis: If the concentration of hydrocloric acid is increased, the rate of reaction will increase and the volume of gass will increase.
The reasoning behind the hypothesis is that when there are more molecules in the solution the reactants collide more often, so more product is made in a shorter periode of time. The equation was: Mg + 2HCl → MgCl2 + H2
Independent variable | Dependent variable | Controled variables | Value | How to control the CV |
Concentration of acid | Rate of...

...An investigation in to the rate of reaction
Plan:
I am going to investigate the rate of reaction. The reaction I will be using is:
Calcium Carbonate + Hydrochloric acid ---- Calcium Chloride + water + carbon dioxide.
CaCO3 + 2HCl ---- CaCl +H2O + CO2
Measurements and Variables:
The variables I have chosen to change is strength of the hydrochloric acid which will be 1 mole, 0.7 mole, 0.5 mole, 0.3 mole and 0.1 mole some variable I will not be using are temperature, mass, density.
The measurements I will be using are time (s) and volume in (cm3).
Fair Test:
To make sure this a fair test I will get exact amounts of the Hydrochloric acid and Calcium Carbonate. I will also make sure that the Gas syringe is at zero when I start the experiment. I will also try and start the stopwatch as soon as I add the Hydrochloric acid.
Safety:
To make sure this will be a safe experiment I will make sure I wear goggles at all time. I will wash my hand immediately after the experiment is over, and will make sure I am attentive when handling acid.
Prediction:
I predict that the stronger the concentration of hydrochloric acid the more carbon dioxide is given off. I think this because there will be more particles in a certain area (15cm3) so there will be more collisions. I also think that there will be a quantitative relationship that if you double the concentration the rate...

...Factors Affecting Rates of Reaction
Thanks to Michelle Craig
Manitoba Curriculum
Chemistry Grade 12; Kinetics, Topic 3-08
Objectives
To design short experiments to investigate and explain qualitatively using collision theory the relationship between reactionrate and temperature, concentration, catalyst, and surface area.
Apparatus and Materials Available
3 x 250 mL beakers magnesium ribbon (1 cm)
3 x test tubes magnesium powder
test tube rack mossy zinc
10 mL graduated cylinder copper turnings
3 x Alka Seltzer® tablets copper(II) sulfate
0.1 M hydrochloric acid, HCl hot bath
1.0 M hydrochloric acid, HCl ice bath
6.0 M hydrochloric acid, HCl steel wool
pieces of zinc (1 cm x 1 cm) thermometer
*additional materials may be made available upon request*
Part 1: Affect of Temperature
Designing an Experiment
A) Design a simple experiment using the reaction of Alka Seltzer® with water that will qualitatively investigate the affect of temperature on the rate of reaction. You may use any of the materials listed above in your investigation. Keep in mind that, in any experiment where you want to determine the affect of one variable, you should attempt to keep all other variables constant.
Write out the steps to your procedure in point form. Be sure to include the details of what...

...Aim:
The rate at which a reaction occurs, or takes place, is affected by various factors, such as the temperature at which the experiment is conducted in, the pressure which is given, the surface area which is exposed, use of catalysts, and the concentration. In this investigation, I would be investigating the affect of surface area, or particle size, in the rate at which a reaction occurs.
Background Information:
The more finely divided the solid is, the faster the reaction happens. A powdered solid will normally produce a faster reaction than if the same mass is present as a single lump. The powdered solid has a greater surface area than the single lump.
Note: Why normally? What exceptions can there be?
Imagine a case of a very fine powder reacting with a gas. If the powder was in one big heap, the gas may not be able to penetrate it. That means that its effective surface area is much the same as (or even less than) it would be if it were present in a single lump.
A small heap of fine magnesium powder tends to burn rather more slowly than a strip of magnesium ribbon, for example.
Imagine a reaction between magnesium metal and a dilute acid like hydrochloric acid. The reaction involves collision between magnesium atoms and hydrogen ions.
How does surface area affect a chemical reaction?
If one of the reactants is a...

...The Rate of a Reaction The area of chemistry that deals with the rate or speed of chemical reactions is known a chemical kinetics. The word “kinetic” is derived from the Greek name kinitikos that means movement or motion. In the present context, the kinetic means the reactionrate or rate of a reaction that is defined as the change in concentration of a reactant or a product with time (M/s). Chemical reaction can be represented by the following general equation. Reactants Products
It is very important for you to understand the meaning of the above equation, which tells us that, during the course of a reaction, the reactant molecules are used up and product molecules are formed. The arrow between the reactants and products indicates the direction of the reaction. Let us represent reactant molecules by A and product molecules by B. Then we can re-write the above equation in the following from: A B (1)
This is a very simple reaction where A molecules are converted into B molecules or one mole of A disappears for each mole of B forms. As the time progresses, the number A molecules decrease and B molecules increase that is shown in the following figure.
100 80 No. of molecules B molecules 60 40 20 0 0 2 4 Time 6 8 10 A molecules
When we say “rate”, it usually means the change...

...reactionrates and concentration (research paper) By katie prestage
what are reactionrates?
The rate of reaction is the speed in which a reaction takes place. This can be measured by the rate in which a reactant is used up, or the rate a product is created. If a reaction has a low rate, it means that the particles are combining at a slow speed. If the rate is high, it means that the particles are coming together at a fast speed. For example, the rusting of iron through oxidation has a slow reactionrate that can take a very long time, but the combustion of cellulose within a fire has an incredibly fast reactionrate taking place in a fraction of a second. Chemical reactions can only take place if particles that are reactants collide with enough energy. The more often particles collide, and the larger the amount of collisions occurring with enough energy, the higher the rate of reaction.
There are a few factors that affect the rate of reaction:
• Concentration - increasing the concentration increases the probability of collision of the reactants. The collision theory, the idea that as more collisions occur in a system there will be more combinations of particles bouncing into...

...﻿Erin Bolton
Chemistry Lab Report
April 29, 2015
Lab: ReactionRates
Introduction: In this experiment we studied the reaction of potassium persulfate, K2S2O8, with potassium iodide, KI. All chemical reactions have an energy barrier to overcome before the reaction will proceed. We will record data based on the concentration, temperature and catalyst for each experiment. Once this has been completed it will be graphed.
Procedure: Due to the chemicals being used having hazard gloves are used for the entire procedure. For this lab the materials we used were pipettors and tips, 10 mL graduated cylinders, large test tubes, test tube racks, corks and timers. The larger test tubes allowed for easier mixing of solutions. The first procedure was a concentration study. The concentration allowed for 9 separate trials. A solution table was provided to ensure proper measurements for each of the trials. The pipettors were used to obtain the appropriate amount of each chemical in order to perform the separate trials. Solution A contained; water, 0.3M potassium iodide, 0.4% starch and 0.02M sodium Thiosulfate. Solution B contained 0.1M Potassium Persulfate. Once all of the solutions were measured out. We individually added solution B to solution A, put the cork in the test tube and the timer was started immediately. We then inverted each solution twice. Once inverted we held a white...